# Problem: How many mL of 0.024 M HCIO 4 would be required to reach the equivalence point in a titration of 32.00 mL of 0.017 M Ca(OH)2?A. 22.67 mLB. 45.33 mLC. 32.00 mLD. 11.33 mLE. 16.00 mL

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###### FREE Expert Solution

We’re being asked to calculate the volume (in mL) of 0.024 M HClO4 (strong acid) required to reach the equivalence point in a titration of 32.00 mL of 0.017 M Ca(OH)2 (strong base)

Recall that at the equivalence point of a titration:

Also, recall that moles = molarity × volume

This means:

$\overline{){\left(\mathbf{MV}\right)}_{{\mathbf{acid}}}{\mathbf{=}}{\left(\mathbf{MV}\right)}_{{\mathbf{base}}}}$

###### Problem Details

How many mL of 0.024 M HCIO 4 would be required to reach the equivalence point in a titration of 32.00 mL of 0.017 M Ca(OH)2?

A. 22.67 mL
B. 45.33 mL
C. 32.00 mL
D. 11.33 mL
E. 16.00 mL